An aqueous solution of an unknown solid salt was placed into fivedifferent test tubes. Into each test tube a couple of drops of differentindicators were then added to each test tube and the color of theindicator in the solution was recorded as shown below. What is theapproximate pH of the solution?TestpHAcidBaseColor in UnknownIndicatortubeRange ColorColorSolution3.0 -1Methyl orange4.4RedYellowYellow3.0 -Congo RedPurpleRedRed5.0Bromcresol3.8 -YellowBlueBlueGreen5.4Bromthymol6.0 -7.64YellowBlueYellowBlue8.2 -PhenolphthaleinColorless BlueColorless10.04.3O 8.4O 5.26.7

The approximately pH value would be 5.2

An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Acid Base Color in Unknown Test Indicator tube pH Range Color Color Solution 3.0 - Methyl orange 4.4 Red Yellow Yellow 1 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 4 Blue 6.0 - Yellow Blue Yellow 7.6 8.2 - Phenolphthalein 10.0 Colorless Blue Colorless LO

An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Acid Base Color in Unknown Test Indicator tube pH Range Color Color Solution 3.0 - Methyl orange 4.4 Red Yellow Yellow 1 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 4 Blue 6.0 - Yellow Blue Yellow 7.6 8.2 - Phenolphthalein 10.0 Colorless Blue Colorless LO

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Indicators can be used to help approximate the pH of a solution based on the indicator colour. Here is an example of how to word the pH approximation for bromothymol blue. Indicator Colour pH approximation Yellow 6.0 and below Green between 6.0 and 7.6 Blue 7.6 and above A Chemistry experiment is done where the pH of various solutions are tested, using indicators. The colours of indicators are recorded as shown below. Indicator Colour pH approximation orange IV orange Indicator Colour pH approximation thymol blue red Indicator Colour pH approximation alizarin yellow R red
In an acid-base titration experiment, the equivalence point on the titration curve was at a pH of 6.0. Based on this information, which of the following is represents the titration experiment that was conducted? It was a titration conducted between a strong base and strong acid It was a titration conducted between a weak acid and a strong base. It was a titration conducted between a strong acid and a weak base
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
You have an unknown solution whose initial pH is 2.90. Addition of 10 ml of the titrant increased the pH to 4.15. Adding small-volume increments of the titrant causes the pH to increase very slightly. At equivalence point, the pH of the solution is at 8.70. Abrupt increase in pH to 10.00 was observed when 0.1 ml of titrant was added after equivalence point. Addition of few more drops of the titrant just increase the pH even more with no buffering region. Which among the choices best describes the analyte? The analyte is a strong monoprotic acid. The analyte is a weak monoprotic acid. The analyte is a weak monoprotic base. O The analyte is a weak diprotic acid. O The analyte is a weak diprotic base.
The indicator thymol blue has two color transitions as indicated in the table. Thymol Blue Indicator Colors Acid color pH Transition range Base color red 1.2-2.8 yellow yellow 8.0-9.6 blue Select the color expected when thymol blue is added to solutions having the given pH values. pH 1 pH 2 orange O yellow O green orange O yellow blue red green O blue O red pH 6 pH 10
From the following set of titrations choose the three most concordant titres and calculate the average titre value run 1 2 3 4 4 titre (ml) 13.40 13.70 13.85 13.45 13.80
Titration A HCl Titrated with NaOH Volume of NaOH pH 0.0 1.00 5.0 1.18 10.0 1.37 15.0 1.60 20.0 1.95 21.0 2.06 22.0 2.19 23.0 2.38 24.0 2.69 25.0 7.00 26.0 11.29 27.0 11.58 28.0 11.76 29.0 11.87 30.0 11.96 35.0 12.22 40.0 12.36 45.0 12.46 50.0 12.52 Titration B HC2H3O2 Titrated with NaOH Volume of NaOH pH 0.0 2.87 5.0 4.14 10.0 4.56 15.0 4.92 20.0 5.34 21.0 5.46 22.0 5.61 23.0 5.80 24.0 6.12 25.0 8.87 26.0 11.30 27.0 11.56 28.0 11.75 29.0 11.87 30.0 11.96 35.0 12.22 40.0 12.36 45.0 12.46 50.0 12.52 1. Titration A, endpoint pH = Titration B, endpoint pH = 2. pKa or pKb = 3. Ka or…
A student obtains the following data from the Determining the pKa of an Acid-Base Indicator experiment. Using this data, calculate the pKa of the indicator in the fourth solution. Solution Abs. pH 3.4 + HCI 0.054 pH 4.6 + NaOH 0.564 Sample # 1 2 345 actual pH 3.34 3.73 3.96 4.22 4.50 Abs. 0.135 0.214 0.295 0.382 0.460
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solution C2. Effect of a base on the pH of a buffer solution Solution Used Initial pH pH after adding 5 drops of КОН pH after adding additional 5 Change in pH Is the tested solution a buffer? Yes or No drops of КОН Water 6.98 10.25 11.78 0.1 M KCI 6.40 9.78 10.54 solution pH 12 buffer solution 11.98 12.18 12.53 pH 1 buffer solution 2.05 2.34 2.65 étv 3 MacBook Air DII DD 80 888 F11 F9 F10 F8 F6 F7 F3 F4 F5 F1 F2 * # $ &
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